KMnO4 dispensed 28.5ml 26.3ml Moles of KMnO4 5.7E-4 5.26E-4 Moles of C2O42- 1.425E-3 1.315E-3 Table 2: (Second Titration) C2O42- Analysis Sample 1 Sample 2 Molarity of KMnO4 0.02m 0.02m Weight of Sample 0.237g 0.225g Final Buret Reading 4.2ml 4.5ml Initial Buret Reading 0ml 0ml Volume of KMnO4 dispensed 4.2ml 4.5ml Moles of KMnO4 8.4E-5 9.0E-5 Moles of C2O42- 2.1E-4 2.25E-4 Calculations: 1.) 2 KMnO4 + 5 K2C2O4 + 8 H2SO4 = 2 MnSO4 + 10 CO2 + 8 H2O + 6 K2SO4 Find moles of C2O42- Trial 1: KMnO4 =
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(12.01 x 2) + (1.0079 x 6)] = 290.704g/mol Mass of CuCl2= 0.850g Equation for reaction CuCl2 + 2DMSO -> CuCl22DMSO Mole ratio between CuCl2 and CuCl22DMSO = 1:1 Mole of CuCl2 = Mass/ Mr = 0.850/134.45 = 0.00632 moles Since the ratio between CuCl2 and CuCl22DMSO = 1:1‚ mole of CuCl2DMSO is also 0.0063 moles. To find theoretical yield of CuCl2.2DMSO Mass = Mr x mole =290.704 x 0.00632 = 1.837g The actual yield gained is 1.573g The percentage yield = (actual yield/ thereotical yield)
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I. Title: Iron-Copper (II) Chloride Reaction II. Purpose: The purpose of this lab is to see how iron reacts with a copper (II) chloride solution. III. Equipment and Reagents Scoop copper (II) chloride (CuCl2) Beaker Iron (Fe) Wash Bottle water (H2O) Scale Hydrogen chloride (M HCl) Filter Paper IV. Procedure: 1. Obtain a clean‚ dry 250 mL beaker. 2. See teacher to obtain a scoop of CuCl2 in the beaker. 3. Add approximately 50 mL of tap water to
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To go on a journey does not necessarily require one to physically move from one place to another. A journey can happen anywhere‚ and at any time‚ even if you are not moving. An inner journey is to transcend above the physical and temporal world into a spiritual realm. This enables one to look at life attentively and be alert to the lessons learnt from experience. ‘Of Eurydice’ by Ivan Lalic‚ ‘Fax X’ by Gwyneth Lewis‚ ‘Wind in the Willows’ by Kenneth Graham‚ ‘The Road Not Taken’ by Robert Frost‚ ‘The
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values used to calculate the moles of magnesium and oxygen for each trial. The moles of magnesium and oxygen were then averaged (to reduce random error) and these values used to determine the experimental mole ratio for Mg : O. Uncertainties for each value were also calculated. Formula and worked examples for these are shown in table 2 below. Excel was used to graph moles of Mg verses moles of O. The equation for the line of best fit was then used to determine the mole ratio of Mg:O and thus the
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Abstract: Liquid-vapor phase of acetone/chloroform was studied through distilling a series of mixtures with different mole fraction. When the mixtures were boiling‚ their vapor was condensed through a water column and collected in a receiving container. Refractive index was collected for starting mixture‚ distillate and residue for each sample. A boiling temperature versus acetone’s mole fraction was constructed to show the liquid-vapor phase diagram. The boiling temperature of azeotrope was determined
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Purpose: To find number of moles of Fe+3 which react with one mole of NH3OH+ in order to partially balance the equation: NH3OH+ + 2Fe+3 "" ? + 2Fe+2 and to find the missing product. Procedure: H2C2O4 and H2SO4 were titrated with potassium permanganate. The molarity of the permanganate was then found because the molarity of the H2C2O4 and H2SO4 were already known. Then hydroxylammonium chloride and ferric sulfate and water was titrated with known potassium permanganate to get the molarity of the
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(amu) 1 mole f X=atomic mass in grams 1 mole of something = 6.022 x 1023 units of that substance 1 mole of a compound =66.022 x 1023 atoms 6.022 x 1023 amu =1 g 2. What is the mass of 6 atoms of Fe? Answer: 6 atoms of Fe x 55.85 amu÷atom of Fe x 1 g of Fe÷6.022 x 1023 amu = 3. How many atoms does it take to make 1 g of Gold (Au)? Answer: 197.0 g Au =1 mole of Au 1 g of Au=? 1 mole of Au/197 g Au
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(II) Sulfate Purpose: The purpose of this lab is to find out how many moles of water there are in one mole of Copper Sulfate (CuSO x HO) and the percent by mass of water in the hydrate. This will be accomplished by heating a determined mass of the hydrate to remove the water‚ and by measuring the salt left over. Introduction: This laboratory experiment will be done to find out how many moles of HO are present per one mole in the hydrate CuSO. A hydrate is a compound that has a fixed number of
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- Mass of crucible and anhydrous salt (31.39g) = .96g 3. How many moles of water is this?
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